What is the molarity of hydrochloric acid in a solution that contains a #3.65g# mass of #HCl(g)# in #500mL# aqueous solution?

Question

17592 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2017-05-09T06:33:23

#"Molarity"-="Moles of solute"/"Volume of solution"#

And here, #"molarity"=((3.65*g)/(36.5*g*mol^-1))/(500*mLxx10^-3*L*mL^-1)=0.200*mol*L^-1#.

Is the calculation consistent dimensionally?

And thus if it is #0.200*mol*L^-1# with respect to hydrogen chloride, it is #0.200*mol*L^-1# with respect to #H_3O^+#, AND #Cl^-#.

What is the #pH# of this solution?

What is the molarity of hydrochloric acid in a solution that contains a #3.65*g# mass of #HCl(g)# in #500*mL# aqueous solution?